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Revision > Chemistry Flame Test Etc. > Flashcards

Chemistry Flame Test Etc. Flashcards

1
Q

Flame test: Lithium

A

Crimson

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2
Q

Flame test: Sodium

A

Yellow

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3
Q

Flame test: Copper

A

Blue- Green

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4
Q

Flame test: Calcium

A

Orange- Red

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5
Q

Flame test: Potassium

A

Lilac

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6
Q

Soluble salts

All (5)

A 
Lithium 
Sodium 
Potassium
Ammonium 
Nitrates
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7
Q

Common Chloride solutions soluble except (2)

A

Silver

Lead

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8
Q

Common Sulfate solutions soluble except

3

A

Lead
Barium
Calcium

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9
Q

Common hydroxides insoluble except (4)

A

Lithium
Sodium
Potassium
Ammonium

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10
Q

Common carbonates insoluble except (4)

A

Lithium
Sodium
Potassium
Ammonium

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11
Q

Equation for mass (moles)

A

Mass = moles*Mr

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12
Q

Equation for mass (conc)

A

Mass= concentration* volume

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13
Q

Equation for moles (conc)

A

Moles = concentration* volume

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14
Q

Name the 3 displacement reactions

A 
KBr + Cl2 
Clear to yellow
KI + Cl2
Clear to brown
KI + Br2
Yellow to orange/brown
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15
Q

Describe the Halogens (4)

A

Fluorine- pale yellow gas
Chlorine - green gas
Bromine- Brown liquid - brown gas
Iodine- black shiny solid- purple gas when sublimes (no liquid)

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16
Q

Silver Halides precipitates and colours (3)

A

Silver chloride - white
Silver bromide - cream
Silver iodide - yellow

17
Q

Precipitate colour of carbonates (3)

A

Copper carbonate- blue-green
Silver carbonate- yellow
Rest of carbonates- white

18
Q

Precipitate colour of copper iodide

A

White

19
Q

Precipitate colours of lead chloride, bromide and iodide

A

White, white, yellow

20
Q

Precipitate colour of insoluble sulfates

A

White

21
Q

Common bromides soluble except (2)

A

Lead, silver

22
Q

Common iodides soluble except

A

Silver, Lead, Copper

23
Q

Test for chloride ion

A

Add silver nitrate forms a white precipitate

24
Q

Describe metallic bonding

A 
Regularly arranged 
Positive ions
Giant lattice
Sea of delocalised electrons hold it together
Electrostatic forces between metal ions
25
Q

Properties of metallic bonding

A 
Conduct electricity
High BP and MP
Malleable
Shiny
Sonorous 
Insoluble in water (react)
Insoluble in non polar solvents
26
Q

Properties of covalent network bonding

A 
Giant lattice
High MP and BP
Don’t conduct (except graphite)
Insoluble in water 
Insoluble in non polar
27
Q

Properties of ionic

A

High MP and BP
Conduct when molten
Often soluble in water
Insoluble in non polar

28
Q

Properties of macromolecular (DNA, polymers)

A 
Weak intermolecular bonds
Moderate BP and MP
Don’t conduct electricity
Insoluble in water
Sometimes soluble
29
Q

Properties of Simple covalent

A 
Weak intermolecular bonds 
Low BP and MP
Don’t conduct electricity 
Insoluble in water , unless can bond with hydrogen in water 
Insoluble in non polar
30
Q

Describe E isomerism

A

Trans, not on the same side, double bind doesn’t allow rotation, stack better

31
Q

Describe Z isomerism

A

Cis on the same zide, also around double bond which doesn’t allow free rotation

32
Q

Name the 4 structural isomers

A

Chain isomerism- branched
Position isomerism- position of branch
Functional group isomerism- ether or alcohol
Stereoisomerism- E trans , Z cis

33
Q

Standard conditions

A

298K (25 degrees)

1 atmospheric pressure

34
Q

What is the ideal gas equation

A

PV= nRT

P- pressure (kPa)
V- volume (m^3) Divide cm by 1mill
n- number of moles
R- gas constant 
T- temperature in Kelvin
35
Q

Properties of group 7

A 
Less reactive going down
MP and BP increases down 
Most are toxic 
Increase atomic radius 
Increase shielding
Oxidising agents
36
Q

Oxidation states exceptions

A

H2O2- O has -1 and not -2
Hydrogen- state +1 unless with metal
Fluorine- always -1

37
Q

Species containing ate include

A

Oxygen

38
Q

How to test for carbonates

A

Add dilute HCl

CO2 will form, limewater turns cloudy

Revision (30 decks)

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